Solutions and Their Concentrations

Transcription

1 Chapter 8 Solutions and Their Concentrations Solutions for Practice Problems Section 8.3 Student Tetbook page Problem What is the concentration in percent (m/v) of each solution? (a) 14.2 g of potassium chloride, KCl (used as a salt substitute), dissolved in 450 ml of solution (b) 31.5 g of calcium nitrate, Ca(NO 3 ) 2,(used to make eplosives), dissolved in 1.80 L of solution (c) 1.72 g of potassium permanganate, KMnO 4, (used to bleach stone-washed blue jeans), dissolved in 60 ml of solution (a) Find the (KCl) in of solution. (b) Find the (Ca(NO 3 ) 2 ) in of solution. (c) Find the (KMnO 4 ) in of solution. In (a), (b), and (c) the mass solute and a volume of solution are given. (a) Use the formula: Mass/volume percent Mass of solute (g) Volume of solution (ml) The ratio of the mass of dissolved solute in of solution must be the same as the ratio of 14.2 g of KCl in 450 ml of solution. Let represent the mass of dissolved solute in of solution. (b) Mass of solute (g) Volume of solution (ml) Use the formula: Mass/volume percent The ratio of the mass of dissolved solute in of solution must be the same as the ratio of 31.5 g of Ca(NO 3 ) 2 in ml of solution. Let represent the mass of dissolved solute in of solution. (c) Mass of solute (g) Volume of solution (ml) Use the formula: Mass/volume percent Method 2 The ratio of the mass of dissolved solute in of solution must be the same as the ratio of 1.72 g of KCl in 60 ml of solution. Let represent the mass of dissolved solute in of solution. 137

2 (a) Method 1 Percent (m/v) 14.2 g 450 ml 14.2 g 450 ml 3.16% 14.2 g 450 ml The concentration of the solution is 3.16% (m/v) (b) Percent (m/v) 31.5 g 1.75% ml 31.5 g ml The concentration of the solution is 1.75% (m/v) (c) Percent (m/v) 1.72 g 60 ml 1.72 g 60 ml 2.9% 31.5 g ml 1.72 g 60 ml The concentration of the solution is 2.9% (m/v) g 1.75 g 2.9 g (a) The units are correct. Estimating roughly that is about 14, this approimates the given. (b) The units are correct. Estimating roughly that is about 36, this approimates the given (c) The units are correct. Estimating roughly that is about 1.8, this approimates the given. 2. Problem A solution of hydrochloric acid was formed by dissolving 1.52 g of hydrogen chloride gas in enough water to make 24.1 ml of solution. What is the concentration in percent (m/v) of the solution? Find the in of solution. You are given a and a volume of solution. Use the formula: Mass/volume percent Mass of solute (g) Volume of solution (ml) The ratio of the mass of dissolved solute in of solution must be the same as the ratio of 1.52 g of HCl in 24.1 ml of solution. Let represent the mass of dissolved solute in of solution. Percent (m/v) 1.52 g 24.1 ml 1.52 g 24.1 ml 6.31% The concentration of the solution is 6.31% (m/v) g 24.1 ml 6.31 g 138

3 The units are correct. Estimating roughly that is about 1.5, this approimates the given mass of HCl that is given solute. 3. Problem At 25 C, a saturated solution of carbon dioide gas in water has a concentration of 0.145% (m/v). What mass of carbon dioide is present in 250 ml of the solution? Find the mass of CO 2 in 250 ml of a solution of known concentration. You are given a concentration of 0.145% (m/v) and a solution volume of 250 ml. Rearrange the formula for (m/v) percent to solve for mass (m). Substitute the known values. Let represent the mass of dissolved HCl in 250 ml of solution. The ratio of dissolved solute in of solution must be the same as the ratio of the mass of solute,, dissolved in 250 ml of solution. 250 ml (m/v) percent volume of solution 100 % % 250 ml 100 % g 250 ml g The units are correct. Use rounded off values to estimate. 250 is 2.5 times 100; 2.5 times.15 is about 0.38 which is close to the answer. 4. Problem Ringer s solution contains three dissolved salts in the same proportions as they are found in blood. The salts and their concentrations (m/v) are as follows: 0.86% NaCl, 0.03% KCl, and 0.033% CaCl 2. Suppose that a patient needs to receive 350 ml of Ringer s solution by an intravenous drip. What mass of each salt does the pharmacist need to make the solution? Find the mass of each solute in 350 ml of solution. You are given the volume of solution and the (m/v) percent concentration of each component of the solution. Rearrange the formula for (m/v) percent to solve for mass (m). Substitute the known values. Let represent the mass of dissolved solute in 350 ml of solution. The ratio of dissolved solute in of solution must be the same as the ratio of the mass of solute,, dissolved in 350 ml of solution. 139

4 Method 1 (NaCl) mass of NaCl Method 2 (NaCl) 350 ml 0.86 g Method 1 (KCl) mass of KCl Method 2 (KCl) 350 ml 0.03 g Method 1 (CaCl 2 ) mass of CaCl 2 Method 2 (CaCl 2 ) 350 ml g (m/v) percent volume of solution (m/v) percent volume of solution (m/v) percent volume of solution 0.86% 350 ml 0.86 g 0.03% 350 ml 0.03 g 0.033% 350 ml g 3.0 g 350 ml 3.0 g 0.1 g 350 ml 0.1 g 0.12 g 350 ml 0.12 g The units are correct. Approimating the answers, you have 3.5 times of solution and therefore there should be about 3.5 times the as is found in. This appears to be the case. Solutions for Practice Problems Student Tetbook page Problem Calculate the mass/mass percent of solute for each solution. (a) 17 g of sulfuric acid in 65 g of solution (b) g of sodium chloride dissolved in 92.2 g of water Hint: Remember that a solution consists of both solute and solvent. (c) 12.9 g of carbon tetrachloride dissolved in 72.5 g of benzene In each of (a), (b), and (c) you must calculate the in of solution. (a) You are given a and a mass of solution. (b) You are given a and a mass of solvent (c) You are given a and a mass of solvent Use the formula: mass/mass percent mass of solution Let the in of soltion be represented by. Equate the ratio of the given in the mass of solution to the ratio of the unknown mass of solute,, in of solution. Solve for. (a) percent (m/m) 17 g 65 g 17 g 65 g 26% sulfuric acid 17 g 65 g 26 g sulfuric acid 140

5 Therefore the percent (m/m) sulfuric acid is 26% (b) mass of solution + mass of solvent g g g percent (m/m) g g sodium chloride g Therefore the percent (m/m) sodium chloride is 16.61% g g g g g Therefore the percent (m/m) sodium chloride is 16.61% (c) mass of solution + mass of solvent 12.9 g g 85.4 g percent (m/m) 12.9 g 15.1% carbon tetrachloride 85.4 g 12.9 g 12.9 g 85.4 g 85.4 g Therefore the percent (m/m) carbon tetrachloride is 15.1% 15.1 g The units in each answer are correct and the final answer has the correct number of significant figures. The magnitude of the answer seems reasonable. 6. Problem If 55 g of potassium hydroide are dissolved in of water, what is the concentration of the solution epressed as mass/mass percent? Find the in of solution. You are given the and the mass of solvent. Use the formula: mass/mass percent mass of solution Let the in of solution be represented by. Equate the ratio of the given in the mass of solution to the ratio of the unknown mass of solute,, in of solution. Solve for. mass of solution + mass of solvent 55 g g percent (m/m) 55 g 35% potassium hydroide 155g 55 g 55 g 35 g 155 g 155 g Therefore the mass/mass percent potassium hydroide is 35% 141

6 The units divide out properly and the correct number of significant figures appear in the final answer. Approimating, 55 is about 1 of 155. The answer seems 3 reasonable. 7. Problem Steel is an alloy of iron and about 1.7% carbon. It also contains small amounts of other materials, such as manganese and phosphorus. What mass of carbon is needed to make a 5.0 kg sample of steel? Find the mass of carbon in a given mass of steel. You are given the mass of steel and the percent by mass of carbon in the steel. Rearrange the formula mass/mass percent mass of solution to find mass. Let the mass of carbon in g of steel be represented by. Equate the ratio of the unknown mass of carbon in the g of steel to the ratio of the known mass of carbon, 1.7 g, in of steel. Solve for. 5.0 kg of carbon g carbon mass of carbon 85 g carbon g 1.7 g (m/m) percent mass of solution g g g 85 g The units divide out properly and the final answer has the correct number of significant figures. Approimating, is 50 times times approimately 2 g is which is near the answer that was calculated. The answer seems reasonable. 8. Problem Stainless steel is a variety of steel that resists corrosion. Your cutlery at home may be made of this material. Stainless steel must contain at least 10.5% chromium. What mass of chromium is needed to make a stainless steel fork with a mass of 60.5 g? Find the mass of chromium in a given mass of steel. You know the percent mass/mass of chromium in steel and the mass of steel. Rearrange the formula mass/mass percent mass of solution to find mass. Let the mass of chromium in 60.5 g of steel be represented by. Equate the ratio of the unknown mass of chromium in the 60.5 g of steel to the ratio of the known mass of chromium, 10.5 g, in of steel. Solve for. 142

7 mass of chromium 60.5 g 10.5 g (m/m) percent mass of solution 10.5% 60.5 g 6.35 g chromium Therefore the mass of chromium is 6.35 g 10.5 g 60.5 g 6.35 g chromium The units in the final answer divide out correctly and the correct number of significant figures are in this answer. 10% of 60 is 6 g which is approimately the answer. This answer seems to be reasonable. 9. Problem 18-carat white gold is an alloy. It contains 75% gold, 12.5% silver, and 12.5% copper. A piece of jewelry, made of 18-carat white gold, has a mass of 20g. How much pure gold does it contain? Find the mass of pure gold present in 20 g of white gold. You know the mass of white gold and the percent mass/mass of gold in white gold. Rearrange the formula mass/mass percent mass of solution to find mass. Let the mass of gold in 20 g of white gold be represented by. Equate the ratio of the unknown mass of gold in the 20 g of white gold to the ratio of the known mass of gold, 75 g, in of white gold. Solve for. (m/m) percent mass of solution mass of pure gold 75 g 20 g 15 g pure gold 20 g 75 g 75 g 20 g 15 g pure gold Therefore the mass of pure gold in 20 g of white gold is 15 g The units divide out correctly and the final answer has the correct number of significant figures. 3 of 20 is 15. The answer seems to be reasonable. 4 Student Tetbook page Problem 60 ml of ethanol is diluted with water to a final volume of 400 ml. What is the percent by volume of ethanol in the solution? Find the volume of ethanol in of ethanol solution. 143

8 You know a volume of ethanol and a volume of ethanol solution. Plan a Strategy Use the formula volume/volume percent volume of solute volume of solution Let the volume of pure ethanol in of solution be represented by. Use ratios to solve for the unknown volume. (v/v) percent 60 ml 400 ml 15% ethanol 60 ml 60 ml 15 ml 400 ml 400 ml Therefore the (v/v) percent ethanol is 15% The units divide out and the final answer has the correct number of significant figures. 15% of 400 is 60. The answer is reasonable. 11. Problem Milk fat is present in milk. Whole milk usually contains about 5.0% milk fat by volume. If you drink a glass of milk with a volume of 250 ml, what volume of milk fat have you consumed? Find the volume of milk fat in a given volume of whole milk. You know the volume/volume percent of milk fat in whole milk and the volume of the milk. Rearrange the formula, volume of solute volume of solution v/v percent to find the volume of solute. Let the volume of milk fat be represented by. Use ratios to solve for the unknown volume. volume of ethanol 5.0 ml 250 ml 5.0 ml (v/v) percent volume of solution 5.0% 250 ml 250 ml 12.5 ml or 12 ml Therefore the volume of milk fat in 250 ml of whole milk is 12 ml. 12 ml The units divide our correctly and the correct number of significant figures are in the final answer. The answer seems reasonable. 144

9 12. Problem Both antifreeze (shown in figure 8.18) and engine coolant contain ethylene glycol. A manufacturer sells a concentrated solution that contains 75% (v/v) ethylene glycol in water. According to the label, a 1:1 miture of the concentrate with water will provide protection against freezing down to a temperature of 37 C. A motorist adds 1 L of diluted solution to a car radiator. What is the percent (v/v) of ethylene glycol in the diluted solution? Find the volume of ethylene glycol in of antifreeze. You know the volume/volume percent concentration of the antifreeze and the volume of diluted solution. Calculate the volume of ethylene glycol in 500 ml of antifreeze. This volume of ethylene glycol will be in of diluted 1:1 antifreeze. volume of ethylene glycol in 500 ml of antifreeze ml ml volume/volume percent volume of ethylene glycol volume of antifreeze ml 1000 ml 38% ethylene glycol ml The answer seems reasonable. If a solution is diluted 1:1, its concentration should be cut in half. 13. Problem The average adult human body contains about 5 L of blood. Of this volume, only about 0.72% consists of leukocytes (white blood cells). These essential blood cells fight infection in the body. What volume of pure leukocyte cells is present in the body of a small child, with only 2.5 L of blood? Find the volume of leukocytes in 2.5 L of blood. The volume of blood and the (volume/volume) percent of leukocytes. The (volume/volume) percentage of leukocytes in blood is assumed to be constant at 0.72%. Let the volume of leukocytes be and solve this ratio for. 2.5 L L L or 18 ml The answer seems reasonable based upon the given (v/v) percent concentration. 14. Problem Vinegar is sold as a 5% (v/v) solution of acetic acid in water. How much water should be added to 15 ml of pure acetic acid (a liquid at room temperature) to make 145

10 a 5%(v/v) solution of acetic acid. Note: Assume that when water and acetic acid are mied, the total volume of the solution is the sum of the volumes of each. Find the volume of water that must be added to a given volume of pure acetic acid to make the concentration 5% (v/v). The volume of pure acetic acid and the final (v/v) percent concentration are known. Let the volume of water that must be added be represented by. The final volume of the solution will be the volume of pure acetic + volume of water (). Use the formula for the (v/v) percent concentration of a solution to solve for. volume/volume percent 15 ml 5% + 15 ml 285 ml or ml volume of solute volume of solution The final answer has the correct unit and number of significant figures. In round numbers, 5% of 300 is close to the calculated answer. This answer seems to be reasonable. 15. Problem Symptoms of mercury poisoning become apparent after a person has accumulated more than 20 mg of mercury in the body. (a) Epress this amount as parts per million for a 60 kg person. (b) Epress this amount as parts per billion. (c) Epress this amount as a (m/m) percent. (a) Epress a mass of 20 mg mercury in a 60 kg person as ppm. (b) Epress a mass of 20 mg of mercury in a 60 kg person as ppb. (c) Epress a mass of 20 mg of mercury in a 60 kg person as (m/m) percent. You know the mass of mercury and the mass of the person. (a) Assume that the mercury is spread out in the body as a solute in a solution. Apply the formula for concentration in parts per million. parts per million mass of solution 106 (b) Apply the relationship that 1 ppb ppm (c) Apply the formula (m/m) percent mass of solution (a) ppm 1g 20 mg Hg mg 60 kg g kg ppm (b) ppb ppm 0.33 ppm ppb (c) (m/m)percent 1g 20 mg Hg mg 60 kg g kg % The answers have the correct units and significant figures and seem reasonable. 146

11 16. Problem The use of the pesticide DDT has been banned in Canada since 1969 because of its damaging effect on wildlife. In 1967, the concentration of DDT in an average lake trout, taken from Lake Simcoe in Ontario, was 16 ppm. Today it is less than 1 ppm. What mass of DDT would have been present in a 2.5 kg trout with DDT present at 16 ppm? Find the mass of DDT in a 2.5 kg fish. The concentration of DDT in ppm and the mass of the fish are given. Assume that the DDT is spread evenly through the fish as a solute in a solution. Rearrange the formula: ppm mass of solution 106 to calculate the 2.5 kg 2500 g mass of DDT ppm mass of fish ppm g g The final has the correct unit and number of significant figures. Estimating with power of ten notation gives this approimate answer. This answer seems reasonable. 17. Problem The concentration of chlorine in a swimming pool is generally kept in the range of 1.4 to 4.0 mg/l. The water in a certain pool has 3.0 mg/l of chlorine. Epress this value as parts per million. (Hint: 1 L of water has a mass of 1000 g) Determine the concentration of chlorine in the water as ppm. The mass of water and the concentration in mg/l are given. Use the formula: ppm mass of solution mg/l g 1L of water has a mass of 1000 g 1g mg ppm g ppm g The final answer has the correct unit and number of significant figures. Estimating with power of ten notation gives this answer. The answer is reasonable. 18. Problem Water supplies with dissolved calcium carbonate greater than 500 mg/l are considered unacceptable for most domestic purposes. Epress this concentration in parts per million. Find the concentration of dissolved calcium carbonate in ppm. The concentration in mg/l is given. 147

12 Use the formula: ppm mass of solution mg g 1 L of water has a mass of g 1g mg ppm g ppm g The final answer has the correct unit and number of significant figures. Estimating with power of ten notation gives this answer. The answer is reasonable. 19. Problem What is the molar concentration of each solution? (a) 0.50 mol of NaCl dissolved in 0.30 L of solution (b) mol of iron(iii) chloride, FeCl 3, dissolved in 120 ml of solution (c) mol of copper(ii) sulfate, CuSO 4, dissolved in 70 ml of solution (d) 4.63 g of sugar, C 12 H 22 O 11, dissolved in 16.8 ml of solution (e) 1.2 g of NaNO 3 dissolved in 80 ml of solution For each of (a), (b), (c), (d), and (e) find the concentration in mol/l. For (a), (b), and (c) the number of moles of solute and the total volume of solution are given. For (d) and (e) the and the total volume of solution are given. If necessary, convert the volume of solution from ml to L. For (a), (b), and (c) use the formula: concentration amount of solute (mol) volume of solution (L) For (d) and (e) find the number of moles of solute and use the above formula. (a) C n 0.50 mol 1.7 mol/l NaCl V 0.30 L (b) 120mL 0.120L C n mol 2.41 mol/l FeCl V L 3 (c) 70 ml L C n mol 1.2 mol/l CuSO V L 4 (d) molar mass of C 12 H 22 O g/mol 16.8 ml L 4.63 g C 12 H 22 O 11 1 mol 342 g mol C 12H 22 O 11 C n mol/l sucrose V (e) molar mass of NaNO 3 85 g/mol 80 ml L 1.2g NaNO 3 1 mol mol NaNO 85 g 3 C n mol 0.18 mol/l NaNO V L mol L The answers all have the correct unit and number of significant figures and seem to be reasonable. 20. Problem What is present in each aqueous solution? 148

13 (a) 1.00 ml of mol/l calcium hydroide, Ca(OH) 2, solution (b) 500 ml of mol/l silver nitrate, AgNO 3, solution (c) 2.5 L of 1.00 mol/l potassium chromate, K 2 CrO 4, solution (d) 40 ml of 6.0 mol/l sulfuric acid, H 2 SO 4, solution (e) 4.24 L of mol/l ammonium nitrate, NH 4 NO 3, solution Find the present in each solution. In each case a concentration in mol/l and a volume are given. Plan a Strategy Where necessary, convert the volume of solution given in ml to L. Rearrange the formula, C n to find the moles of solute and change this to grams. V (a) n C V mol/l 1.00 L mol molar mass of Ca(OH) 2 74 g/mol mol Ca(OH) 2 74 g 3.3 g Ca(OH) 1 mol 2 (b) 500 ml L n C V mol/l L mol molar mass of AgNO g/mol mol 170 g 8.50 g AgNO mol 3 (c) n C V 1.00 mol/l 2.5 L 2.5 mol molar mass of K 2 CrO g/mol 2.5 mol K 2 CrO g gk mol 2 CrO 4 (d) 40.0 ml L n C V 6.0 mol/l L 0.24 mol H 2 SO 4 molar mass of H 2 SO 4 98 g/mol 0.24 mol H 2 SO 4 98 g 24 g H mol 2 SO 4 (e) n C V mol/l 4.24 L 3.29 mol NH 4 NO 3 molar mass of NH 4 NO g/mol 3.29 mol NH 4 NO g 263 g NH mol 4 NO 3 In each case the final answer has the correct unit and number of significant figures. These answers are reasonable. 21. Problem A student dissolves g of silver nitrate, AgNO 3, in water to make 500 ml of solution. What is the molar concentration of the solution? Find the concentration of the solution in mol/l You know the mass of silver nitrate, its formula and the volume of solution. Convert the mass of AgNO 3 to moles, the volume of solution from ml to L and use the formula C n to calculate the concentration in mol/l. V 149

14 molar mass of AgNO g/mol g AgNO 3 1 mol g mol AgNO 3 C n V mol L mol/l AgNO 3 The final answer has the correct unit and number of significant figures. This answer is reasonable. 22. Problem What volume of 0.25 mol/l solution can be made using 14 g of sodium hydroide, NaOH? Find the volume of NaOH solution. You know the concentration of the solution and the mass and the formula of the solute. Convert the mass of NaOH to moles and rearrange the formula C n V the volume. molar mass of NaOH 40 g/mol 14 g NaOH 1 mol 0.35 mol NaOH V n C 40 g 0.35 mol 0.25 mol/l 1.4 L to calculate The final answer has the correct unit and number of significant figures and seems reasonable. 23. Problem A bottle of skin lotion contains a number of solutes. One of these solutes is zinc oide, ZnO. The concentration of zinc oide in the skin lotion is mol/l. What mass of zinc oide is present in the bottle? Find the in the bottle of lotion. You know the concentration and formula of the zinc oide and the volume of the solution. Convert the volume of the solution from ml to L and rearrange the formula C n V to find the moles of solute. Convert the moles of solute to grams using the molar mass L n C V mol/l L mol ZnO molar mass of ZnO 81.4 g/mol mol ZnO 81.4 g 7.45 g ZnO mol 150

15 The final answer has the correct unit and number of significant figures and seems reasonable. 24. Problem Formalin is an aqueous solution of formaldehyde, HCHO, used to preserve biological specimens. What mass of formaldehyde is needed to prepare 1.5 L of formalin with a concentration of 10 mol/l? Find a in the formaldehyde solution. You know the concentration and volume of the formalin solution. Rearrange the equation C n to find the moles of solute. Use the molar mass of V formaldehyde to convert this number of moles to grams. n C V 10 mol/l 1.5 L 15 mol HCHO molar mass of HCHO 30 g/mol 15 mol HCHO 30 g/mol g HCHO The final answer has the correct unit and number of significant figures and seems reasonable. 25. Problem Suppose that you are given a solution of 1.25 mol/l sodium chloride in water, NaCl (aq). What volume must you dilute to prepare the following solutions? (a) 50 ml of 1.00 mol/l NaCl (aq) (b) 200 ml of mol/l NaCl (aq) (c) 250 ml of mol/l NaCl (aq) ) Find the volume of the concentrated solution that must be used to prepare the given volume of dilute solution. In each case you know the volume in ml of dilute solution to prepare and the concentrations of the concentrated and the dilute solutions. Convert the volume of the dilute solution from ml to L. The moles of solute in the final dilute solution moles of solute taken from the concentrated solution. apply the relationship: n (NaCl) in concentrated solution n (NaCl) in dilute solution (C V) concentrated (C V) dilute (a) (C V) concentrated (C V) dilute 1.25 mol/l V 1.00 mol/l L V L or 40 ml (b) (C V) concentrated (C V) dilute 1.25 mol/l V mol/l L V L or 128 ml 151

16 (c) (C V) concentrated (C V) dilute 1.25 mol/l V mol/l L V L or 60.0 ml In each case the unit and number of significant figures is correct. The volume of concentrated solution needed is always smaller than the volume of the dilute solution, which is reasonable. 26. Problem What concentration of solution is obtained by diluting 50.0 ml of mol/l aqueous sodium nitrate, NaNO 3 to each volume? (a) 120 ml (b) 400 ml (c) 5.00 L Find the final concentration of a solution after diluting. In each case, you know the volume and the concentration of the concentrated solution as well as the final volume of dilute solution. Convert the volume of concentrated solution from ml to L. Apply the relationship developed in question 25. (C V) concentrated (C V) dilute (a) (C V) concentrated (C V) dilute mol/l L C L C mol/l (b) (C V) concentrated (C V) dilute mol/l L C L C mol/l (c) (C V) concentrated (C V) dilute mol/l L C 5.00 L C mol/l In each case, the final answer has the correct unit and number of significant figures. The concentration of the diluted solution in each case is less than the concentration of the concentrated solution, which is reasonable. 27. Problem A solution is prepared by adding 600 ml of distilled water to of 0.15 mol/l ammonium nitrate, NH 4 NO 3. Calculate the molar concentration of the solution. Assume that the volume quantities can be added together. Find the final concentration after diluting a solution. You know the initial volume and concentration of the starting (concentrated) solution. Also the volume of water that is added is given so you can determine the final volume of the diluted solution. 152

17 Add the volume of water to the initial volume of the concentrated solution. Apply the previously developed relationship, (C V) concentrated (C V) dilute and solve for the final concentration. final volume of solution 600 ml water + of solution 700 ml L (C V) concentrated (C V) dilute 0.15 mol/l L C L C mol/l The final answer has the correct unit and number of significant figures. The final concentration is less than the initial concentration, which is reasonable. 153